CHEM126 – CHAPTER 18 – REGULAR HOMEWORK / ELECTROCHEMISTRY I

 

CHAPTER 18 REGULAR HOMEWORK:

ELECTROCHEMISTRY I

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Question 1

 

Easy: Complete and balance the following redox reaction in acid solution:

Cl2(g) + Br(aq) → Cl(aq) + Br2(l)

For the balanced oxidation half-reaction, how many electrons are produced? How many bromide ions are there? (Always use smallest integer coefficients.)
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Explanation

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Question 2

 

How many chlorine molecules are in the balanced equation?
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Explanation

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Question 3

 

Medium: Complete and balance the following redox reaction in acid solution:

Cu(s) + NO3-(aq) → NO(g) + Cu2+(aq)

For the balanced reduction half-reaction, how many electrons are needed? How many H+ ions are there?
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Explanation

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Question 4

 

How many H+ ions are in the balanced equation?

(If the H+ ions are the left side (reactant), write it as a positive number. If they are the right side (product), write it as a negative number.)
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Explanation

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Question 5

 

Complete and balance the following redox reaction in acid solution:

MnO4-(aq) + C2H2O4(aq) → Mn2+(aq) + CO2(g)

For the balanced oxidation half-reaction, how many electrons are produced? How many H+ ions are there?
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Explanation

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Question 6

 

How many H+ ions are in the balanced equation?

(If the H+ ions are the left side (reactant), write it as a positive number. If they are the right side (product), write it as a negative number.)
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Explanation

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Question 7

 

Complete and balance the following redox reaction in basic solution:

ClO(aq) + CrO2-(aq) → Cl(aq) + CrO42-(aq)

For the balanced oxidation half-reaction, how many electrons are produced? How many OH- ions are there?

Hint given in the general feedback.

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Explanation

Balance the half reaction as if it were in acid. Next neutralize the Hby adding OH.

Question 8

 

How many OH- ions are in the balanced equation?

(If the OH- ions are the left side (reactant), write it as a positive number. If they are the right side (product), write it as a negative number.)
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Explanation

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Question 9

 

Complete and balance the following redox reaction (using smallest coefficients) in basic solution:

Br2(aq) → Br(aq) + BrO3-(aq)

First balance the oxidation half-reaction. How many OH- ions are there in this half-reaction?

(If the OH- ions are the left side (reactant), write it as a positive number. If they are the right side (product), write it as a negative number.)
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Explanation

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Question 10

 

In the balanced reaction, how many Br- ions, OH- ions, and water moleules are there?
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Explanation

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Question 11

 

Complete and balance the following redox reaction in basic solution:

H2O2(aq) + N2H4(aq) → N2(g) + H2O(l)

First balance the reduction half-reaction. How many OH- ions are there in this half-reaction?

(If the OH- ions are the left side (reactant), write it as a positive number. If they are the right side (product), write it as a negative number.)
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Explanation

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Question 12

 

In the balanced reaction, how many N2 molecules, OH- ions, and water moleules are there?

 

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Explanation

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Question 13

 

Calculate Eº from the table of standard potentials (Appendix H p. A-15 (Tro) or Appendix 5 p. A27 (Zumdahl)) for the following reaction:

Zn(s) + Fe2+(aq) → Zn2+ + Fe(s) 

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Explanation

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Question 14

 

Is the reaction spontaneous as written or spontaneous in the reverse direction under standard conditions?
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Explanation

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Question 15

 

Calculate Eº for the following reaction:

AgCl(s) + Fe2+(aq) → Ag(s) + Fe3+(aq) + Cl(aq)

 

 

 

Explanation

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Question 16

 

Is the reaction spontaneous as written or spontaneous in the reverse direction under standard conditions?
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Explanation

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Question 17

 

Calculate Eº from for the following reaction:

Br2(l) + 2Cl(aq) → Cl2(g) + 2Br(aq)
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Explanation

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Question 18

 

Is the reaction spontaneous as written or spontaneous in the reverse direction under standard conditions?
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Explanation

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Question 19

 

Warmup question Which of the following statements are true about a positive electrode in a half-reaction?
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Explanation

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Question 20

 

A half-cell that consists of a copper wire in 1.00 M CuNO3 solution is connected by a salt bridge to a half cell containing a 1.00 M X(II) acetate solution and an electrode of metal X. The voltage of the cell is 1.93 V, with metal X as the positive electrode. Calculate the standard reduction potential for the X half-reaction. The standard reduction potential of the copper half-reaction is 0.52 V. (Hint, write the half-reactions and the overall chemical equation for the spontaneous reaction.)
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Explanation

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Question 21

 

Calculate ΔGo (in J) for 1 moles of electron(s) in each half-reaction and a standard potential of 0.30 V.
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Explanation

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Question 22

 

Calculate ΔGo (in J) for 1 moles of electron(s) in each half-reaction and a standard potential of -0.46 V.
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Explanation

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Question 23

 

Calculate Keq for 2 moles of electron(s) in each half-reaction and a standard potential of 0.45 V.

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Explanation

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Question 24

 

Calculate Keq for 3 moles of electron(s) in each half-reaction and a standard potential of -0.27 V.

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Explanation

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Question 25

 

Calculate the potential for: Zn(s) + Fe2+(aq) → Zn2+(aq) + Fe(s)

when the concentrations of the soluble species are as follows:

[Fe2+] = 0.11 M, [Zn2+] = 0.00097 M

See problem 21, if you don’t want to recalculate the standard potential.

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Explanation

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Question 26

 

Calculate the potential for: AgCl(s) + Fe2+(aq) → Ag(s) + Fe3+(aq) + Cl-(aq)

when the concentrations of the soluble species are as follows:

[Fe2+] = 0.34 M, [Fe3+] = 0.058 M, and [Cl-] = 0.0021 M.

 

 

Explanation

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Question 27

 

Calculate the potential for: Br2(l) + 2Cl-(aq) → Cl2(g) + 2Br-(aq) Use Eº = -.300 V

when the concentrations of the soluble species are as follows:

[Cl-] = 0.44 M, [Br-] = 6.7×10-3 M, PCl2 = 4.1×10-2 atm
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Explanation

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